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Chapter 23: Problem 50

Identify each of the following coordination complexes as either diamagnetic or paramagnetic: (a) \(\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}\) (b) square planar \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}\) (c) \(\left[\mathrm{Ru}(\mathrm{bipy})_{3}\right]^{2+}\) (d) \(\left[\mathrm{CoCl}_{4}\right]^{2-}\)

Short Answer

Expert verified
The coordination complexes can be identified as diamagnetic or paramagnetic as follows: (a) \(\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}\): diamagnetic (b) square planar \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}\): paramagnetic (c) \(\left[\mathrm{Ru}(\mathrm{bipy})_{3}\right]^{2+}\): paramagnetic (d) \(\left[\mathrm{CoCl}_{4}\right]^{2-}\): paramagnetic

Step by step solution

01

Identify the metal ion and oxidation state

First, we need to determine the oxidation state of the metal ion in each complex, as this will help us find the electron configuration. (a) For \(\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}\), the metal ion is Ag in a +1 oxidation state. (b) For the square planar complex \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}\), the metal ion is Cu in a +2 oxidation state. (c) For \(\left[\mathrm{Ru}(\mathrm{bipy})_{3}\right]^{2+}\), the metal ion is Ru in a +2 oxidation state. (d) For \(\left[\mathrm{CoCl}_{4}\right]^{2-}\), the metal ion is Co in a +2 oxidation state (considering the 4 chlorine atoms (charges -1 each), the charge on Co needs to be +2).
02

Determine the electron configuration

Now we will determine the electron configuration for the metal ions based on their oxidation states. (a) Ag in +1 oxidation state has an electron configuration of \([Kr]4d^{10}\). (b) Cu in +2 oxidation state has an electron configuration of \([Ar]3d^9\). (c) Ru in +2 oxidation state has an electron configuration of \([Kr]4d^6\). (d) Co in +2 oxidation state has an electron configuration of \([Ar]3d^7\).
03

Determine if there are unpaired electrons

With the electron configurations, we can now determine if there are unpaired electrons present. (a) \([Kr]4d^{10}\) for Ag in +1: no unpaired electrons (all d-electrons are paired) (b) \([Ar]3d^9\) for Cu in +2: one unpaired electron (1 electron in the d-orbital) (c) \([Kr]4d^6\) for Ru in +2: two unpaired electrons (2 electrons in the d-orbitals) (d) \([Ar]3d^7\) for Co in +2: three unpaired electrons (3 electrons in the d-orbitals)
04

Identify complexes as diamagnetic or paramagnetic

Based on the number of unpaired electrons, we can identify each complex as diamagnetic or paramagnetic. (a) \(\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}\): diamagnetic (no unpaired electrons) (b) square planar \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}\): paramagnetic (one unpaired electron) (c) \(\left[\mathrm{Ru}(\mathrm{bipy})_{3}\right]^{2+}\): paramagnetic (two unpaired electrons) (d) \(\left[\mathrm{CoCl}_{4}\right]^{2-}\): paramagnetic (three unpaired electrons)

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Most popular questions from this chapter

(a) A compound with formula \(\mathrm{RuCl}_{3}\) \(\cdot 5 \mathrm{H}_{2} \mathrm{O}\) is dissolved in water, forming a solution that is approximately the same color as the solid. Immediately after forming the solution, the addition of excess AgNO \(_{3}(a q)\) forms 2 mol of solid AgCl per mole of complex. Write the formula for the compound, showing which ligands are likely to be present in the coordination sphere. (b) After a solution of \(\mathrm{RuCl}_{3}\) \(\cdot 5 \mathrm{H}_{2} \mathrm{O}\) has stood for about a year, addition of \(\mathrm{AgNO}_{3}(a q)\) precipitates 3 mol of AgCl per mole of complex. What has happened in the ensuing time?

Determine if each of the following metal complexes is chiral and therefore has an optical isomer: (a) square planar \(\left[\mathrm{Pd}(\mathrm{en})(\mathrm{CN})_{2}\right],(\mathbf{b})\) octahedral \(\left[\mathrm{Ni}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+},(\mathbf{c})\) octahe- dral \(\operatorname{cis}-\left[\mathrm{V}(\mathrm{en})_{2} \mathrm{ClBr}\right]\)

Generally speaking, for a given metal and ligand, the stability of a coordination compound is greater for the metal in the \(+3\) rather than in the \(+2\) oxidation state (for metals that form stable \(+3\) ions in the first place). Suggest an explanation, keeping in mind the Lewis acid-base nature of the metal-ligand bond.

Carbon monoxide, CO, is an important ligand in coordination chemistry. When \(\mathrm{CO}\) is reacted with nickel metal, the product is \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right],\) which is a toxic, pale yellow liquid. (a) What is the oxidation number for nickel in thiscompound? (b) Given that \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) is a diamagnetic molecule with a tetrahedral geometry, what is the electron configuration of nickel in this compound? (c) Write the name for \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) using the nomenclature rules for coordination compounds.

Which periodic trend is partially responsible for the observation that the maximum oxidation state of the transition-metal elements peaks near groups 7 \(\mathrm{B}\) and 8 \(\mathrm{B} ?\) (a) The number of valence electrons reaches a maximum at group 8 \(\mathrm{B} .\) (b) The effective nuclear charge increases on moving left across each period. (c) The radii of the transition-metal elements reach a minimum for group \(8 \mathrm{B},\) and as the size of the atoms decreases it becomes easier to remove electrons.
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